Search: Ag.Science

Number of results: 48,473

physical science
I suppose this would be 1 mol/??g Ag or ??g Ag/1 mol where ??g Ag stands for the atomic mass of Ag which you can find on the periodic table. I think it is 107.87 but check me out on that.
Thursday, December 4, 2008 at 8:51pm by DrBob222

science- chemistry
What is the concentration of Ag+ in 0.0543M AgNO3 and 1.1657CN-? Ag+ +2CN- <-> [Ag(CN)sub2]- kf = 5.3x10^18
Monday, May 10, 2010 at 12:36am by pigglet

Chemistry
Did you intend Ag/Ag^+ or Ag/Ag^2+. I will assume you intended Ag/Ag^+ Ag^+ + e ==> Ag Eo = 0.80 Fe^2+ ==> Fe^3+ Eo = -0.77 ================== Ag^+ + Fe^2+ ==> Ag + Fe^3+ Eocell = 0.03 Then Ecell = EoCell - (0.0592/n)log Q where Q = (Fe^3+)/(Fe^2+)
Friday, July 20, 2012 at 4:38pm by DrBob222

Chemistry
In the reaction: Cu(s) + 2 Ag+(aq) ---> Cu2+(aq) + 2 Ag(s, the oxidizing agent is ? 1.Cu 2.Cu2+ 3.Ag+ 4.Ag i know its Ag but is it Ag+ or just Ag? what does that extra plus mean?
Sunday, March 20, 2011 at 9:51pm by Alexis

CHem
mol ratio Ag/Cu = 7.8 which means Ag = 7.8*Cu which means that the Ag is whatever the Cu is times 7.8 (Ag is the larger component). OR, said another way, 7.8 mols Ag to 1 mol Cu; then 7.8(107.87)g Ag to 63.546 g Cu. I get %Ag = almost 93% and Cu slightly more than 7% I think ...
Tuesday, September 23, 2008 at 10:16pm by DrBob222

Chemistry
In the reaction: Cu(s) + 2 Ag+(aq) ---> Cu2+(aq) + 2 Ag(s) 1.Cu 2.Cu2+ 3.Ag+ 4.Ag i know its Ag but is it Ag+ or just Ag? what does that extra plus mean?
Sunday, March 20, 2011 at 8:42pm by Alexis

chemistry
AgBr==> Ag^+ + Br^- Ag^+ + 2NH3 ==> Ag(NH3^+ eqn 1..Ksp = (Ag^+)(Br^-) Kf = [Ag(NH3)2^+]/(Ag^+)(NH3)^2 Let S = solubility, then eqn 2..S = (Br^-) = (Ag^+) + [Ag(NH3)2^+] eqn 3..3.9 = (NH3) + (NH4^+) + 2[Ag(MH3)2^+] Three equations as above. 1..as is 2..(Ag^+)&...
Friday, November 4, 2011 at 1:51am by DrBob222

Chemistry
5 moles Ag = 5*atomic mass Ag = ?? grams. But Ag coins are not pure Ag; in fact the percentage varies and some contain no Ag at all. ??grams Ag/percent(as a fraction) = ??grams coins. Then ??g coins/26 = # coins
Sunday, June 26, 2011 at 10:57pm by DrBob222

Chemistry
For the following balanced equation: 2 Ag+ (aq) + Cu(s) Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. 2Ag+(aq) Cu2+(aq) 2Ag(s) Cu(s) B. Cu(s) Cu2+(aq) Ag+(aq) Ag(s) C. Ag+(aq) Cu2+(aq) Cu(s) Ag(s) D. Cu2+(aq) Cu(s) ...
Saturday, May 7, 2011 at 12:49pm by Jessie

Chemistry
Actually, Ag^+ = x (not x^2) if that's what you let it stand for. The squared part of it comes from the Ksp expression which is (Ag^+)^2(CrO4^-2) = 1.1 x 10^-12 (Ag^+)^2 = (1.1 x 10^-12/1.0 x 10^-4) = (Ag^+) = sqrt of ........... (Ag^) = 1.05 x 10^-4 but you are allowed ...
Monday, August 10, 2009 at 4:48pm by DrBob222

chemistry
For the following balanced equation: 2 Ag+ (aq) + Cu(s) Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s) Cu2+(aq) Ag+(aq) Ag(s) B. Cu2+(aq) Cu(s) Ag(s) Ag+(aq) C. Ag+(aq) Cu2+(aq) Cu(s) Ag(s) D. 2Ag+(aq) Cu2+(aq...
Friday, April 18, 2008 at 9:57pm by Matt

chem
a) q = mass Ag x specific heat Ag x (Tf - Ti) You have mass Ag, sp. H. Ag, and Tf (final T) and Ti (initial T). Solve for q. b) You have specific heat Ag which is the energy required to raise 1 g Ag by 1 degree C. 0.24 J/g*c x (107.87 g Ag/mol) = ??
Monday, November 26, 2007 at 1:41pm by DrBob222

Chemistry
I think the equations you want are as follows: AgI(s) ==> Ag^+ + I^- Ksp = (Ag^+)(I^-) = look up. Ag^+ + 2CN^- ==> Ag(CN)2^- Kf = [Ag(CN)2^-]/(Ag^+)(CN^-)^2 = look up.
Monday, May 11, 2009 at 9:17pm by DrBob 222

Chemistry
A voltaic cell is constructed as follows: Ag(s)|Ag^+,(satd Ag2CrO4)||Ag^+(0.110 M)|Ag(s). What is the value of Ecell? For Ag2CrO4, Ksp=1.1*10^-12.
Saturday, March 28, 2009 at 10:45pm by Daniel

chemistry
Balance the following redox equation occurring in a basic solution: AG + CN{-} + O2 = AG(CN)2{-} I tried...but this is wrong...2H2O+ AG + CN{-} + O2 = AG(CN)2{-}+4OH{-}... I am supposed to do half reactions...how do I spit the product AG(CN)2{-}?????
Wednesday, April 27, 2011 at 6:18pm by lili

Chemistry
For the following balanced equation: 2 Ag+ (aq) + Cu(s) ---> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu2+(aq)/ Cu(s) // Ag(s) / Ag+(aq) B. 2Ag+(aq)/ Cu2+(aq)// 2Ag(s)/ Cu(s) C. Ag+(aq) / Cu2+(aq)// Cu(s...
Thursday, May 8, 2008 at 2:34am by Amy

Chemistry
For the following balanced equation: 2 Ag+ (aq) + Cu(s)--> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s)/Cu2+(aq)//Ag+(aq)/Ag(s) B. Cu2+(aq)/ Cu(s)// Ag(s)/ Ag+(aq) C. Ag+(aq)/ Cu2+(aq)// Cu(s)/ Ag(s) D...
Friday, April 18, 2008 at 10:14pm by Matt

UCI Chemistry Webworks
For the following balanced equation: 2 Ag+ (aq) + Cu(s) <<->> Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. 2Ag+(aq) | Cu2+(aq) || 2Ag(s) | Cu(s) B. Cu(s)| Cu2+(aq) || Ag+(aq) | Ag(s) C. ...
Saturday, May 7, 2011 at 10:14pm by Tom

Chemistry
you add 0.05ml of 0.10M agno3 to 4ml of 2.0 nacl it forms saturated solution of agcl<---> ag+ + cl- using a saturated solution you set up ag | ag+( test solution after reaction) || ag+(1.0ml) | ag how do we calc the equilibrium of ag+ of the test solution after ...
Wednesday, March 30, 2011 at 12:36am by Jeanine

chemistry
you add 0.05ml of 0.10M agno3 to 4ml of 2.0 nacl it forms saturated solution of agcl<---> ag+ + cl- using a saturated solution you set up ag | ag+( test solution after reaction) || ag+(1.0ml) | ag how do we calc the equilibrium of ag+ of the test solution after ...
Tuesday, March 29, 2011 at 7:04pm by Jeanine

Chemistry
1.Write the equations for AgCl, Ag(NH3)2, and NH3. For example, AgCl ==> Ag^+ + Cl^-, Ag^+ + 2NH3 ==> Ag(NH3)2^+ , and the NH3 + H2O ==> NH4^+ + OH^- 2. Write the Ksp for AgCl, Kb for NH3, and Kformation for Ag(NH3)2. 3. Solubility AgCl = (Cl^-) = (Ag...
Sunday, April 5, 2009 at 6:51pm by DrBob222

Chemistry
For the following balanced equation: 2Ag+(aq) + Cu(s)<->Cu2+ (aq) + 2 Ag(s) Which letter corresponds to the correct cell notation at standard state conditions? A. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) B. Ag+(aq) | Cu2+(aq) || Cu(s) | Ag(s) C. 2Ag+(aq) | Cu2+(aq...
Monday, April 21, 2008 at 2:16am by David

science
1 mole of Ag = 108 g So, 5g = 5/108 = 0.0463 moles Ag Each mole of propanol produces 1.5 moles Ag, so each mole of Ag requires 2/3 moles of propanol (sorry for the 3/2 typo above). 2/3 * .0463 = 0.0309 moles of propanol required. mol wt of propanol is 58g, so you need 1.79 g
Thursday, January 31, 2013 at 9:39am by Steve

Inorganic chemistry
Calculate the standard reduction potential for the following reaction at 25 degrees Celsius Ag(NH3)2^+(aq) +e^- ==> Ag(s) + 2 NH3(aq) given the following thermodynamic information Ag^+(aq) + e^- ==>Ag(s) E naught = 0.799V Ag^+(aq) + 2NH3(aq) ==> Ag(NH3)2...
Saturday, April 11, 2009 at 10:18pm by Steve

chemestry
Two or three things I want to point out to you. First, note the correct spelling of chemistry. Second, Au is NOT soluble in HNO3 alone. That's why Au is called a noble metal and it requires aqua regia (royal water) to dissolve it. Aqua regia is a mixture of HNO3 and HCl. ...
Thursday, September 29, 2011 at 1:16pm by DrBob222

Inorganic chemistry
The following electrochemical cell has the potential of +0.617V at 25 degrees Celsius Pt ! H2(g, 1.00 atm) ! H+ (aq, 1.00M !! Ag^+(aq) ! Ag The standard reduction potential, E naught, of Ag^+ = 0.799V. What is the Ag+ concentration?
Saturday, April 11, 2009 at 11:15pm by Steve

Chemistry
I would pick A. B no, Mg reacts with H2O. C no, It's Ag^+, not Ag^2+ D no, there is no Ag^2+ swolid E no, should be Zn2+(aq)|Zn(s)
Monday, May 21, 2012 at 12:53pm by DrBob222

chemistry
Silver has two naturally occurring isotopes (Ag-107 and Ag-109). (a) Use the periodic table to find the atomic mass of silver. (b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109? (c) If the mass of Ag-107 is 106.905, what is the mass of ...
Monday, September 27, 2010 at 12:05pm by NEED HELP

chemistry
AgI ==> Ag^+ + I^- Ksp = (Ag^+)(I^-) Ag^+ = x I^- = x solve for x.
Thursday, November 4, 2010 at 4:08pm by DrBob222

chemistry
moles AgBr = grams/molar mass. moles Ag = same since there is 1 Ag in 1 AgBr. grams Ag = moles Ag x molar mass Ag %Ag = (mass Ag/mass sample)*100 = ??
Thursday, October 28, 2010 at 5:39pm by DrBob222

Inorganic chemistry
I do not know how I should approach this problem either. The following electrochemial cell has a potential of+0.617V at 25 degrees Celsius Pt ! H2(g,1.00atm) ! H^+(aq,1.00M) !! Ag^+(aq) ! Ag The standard reduction potential ,E naught of Ag^+ = 0.700V. What is the Ag^+ ...
Tuesday, April 14, 2009 at 5:28pm by Steve

chemistry
Silver is electroplated at the cathode of an electrolysis cell by 1/2 reaction Ag(aq) + e- --> Ag(s). How many moles of electrons are required to electroplate 5.8g of Ag?
Wednesday, November 30, 2011 at 8:17am by Ashley

Chemistry
The extra plus means the ion. You could write the half reaction for the Ag this way. Ag(s) ==> Ag+ + e which means the Ag is losing an electron to become the silver +1 ion.
Sunday, March 20, 2011 at 9:51pm by DrBob222

chemistry
Use PV = nRT and solve for n = number of mols H2S at the conditions listed. Then convert mols H2S to mols Ag using the coefficients in the balanced equation. Finally, g Ag = mols Ag x atomic mass Ag.
Tuesday, July 24, 2012 at 7:13pm by DrBob222

chemistry
an electrochemical cell uses Al and Al+3 in one compartment and Ag and Ag+ in the other write a balanced equation for the rxn that will occur spontaneously in this cell would that just be Al + Al+3 + 2e --> Ag + Ag+ ?
Sunday, January 18, 2009 at 5:46pm by erin

Chemistry Check
1) Cd | Cd(NO3)2 || Ag(NO3)2 | Ag Reduction at Cathode: [Ag+ + e- ---> Ag]x2 Oxidation at Anode: Cd ---> Cd2+ + 2e- 2Ag+ + Cd ---> Ag + Cd2+ Is this right? 2IO3- + 12H+ + 5Zn ---> I2 + 6H2O + 5Zn2+
Wednesday, March 5, 2008 at 9:35pm by Alex

chemistry
Silver is electroplated at the cathode of an electrolysis cell by the half reaction Ag+(aq) + e- --> Ag(s) How many moles of electrons are required to electroplate 5.8g of Ag?
Friday, November 25, 2011 at 11:02pm by Monique

Chemistry
2.99 g AgCl x (atomic mass Ag/molar mass AgCl) = about 2.25g Ag but you need to confirm that. Then % Ag =(mass Ag/mass sample)*100 = ? Approx 90%; BUT that must be an old dime. The new ones don't have that much.
Monday, October 29, 2012 at 10:04am by DrBob222

science
looks like each mole of propanol produces 2 moles of Ag. If the reaction yields 75%, then each mole of propanol produces 1.5 moles Ag. So, how many moles of Ag in 5g? 3/2 that of propanol, convert to g.
Thursday, January 31, 2013 at 9:39am by Steve

Chemistry
The iron half cell is Fe(s) ==> Fe^2+(aq) + 2e The Ag half cell is Ag^+(aq) + e ==> Ag(s) Overall is Fe(s) + 2Ag^+(aq) ==> Ag(s) + Fe^2+(aq) I have written (aq) just to show Ag or Fe is in solution; the usual procedure is to place the concn in M there. The...
Friday, June 17, 2011 at 1:55pm by DrBob222

Chemistry
Hi I need help with another balancing oxidation-reduction reaction: Cu(s) + Ag^1+(aq) → Cu^2+(aq) + Ag(s) My work: Cu (s) --> Cu^2+ (aq) + 2e- 2 [1e +Ag^1+ (aq) --> Ag(s)] Cu(s) + 2 Ag(aq) --> Cu (aq) + 2 Ag (s) Is this right? And I need help ...
Sunday, May 16, 2010 at 5:30pm by Anonymous

Chemisty
How many grams of sodium bicarbonate mut be decomposed by: HCl (ag) + NaHCO3 (ag) ----> NaCl (ag) + CO2 (g) + H2O (l) to yield 75.0 mL of carbon dioxide at STP?
Saturday, April 23, 2011 at 2:13pm by Adele

Science
What are the theoretical molar ratio values for Ag:Cu and Ag:AgNO3? Compare these values to the values you got in your experiment and compute a percent error for your work.
Friday, May 27, 2011 at 1:27am by Christine

chemistry
I'll do the first one for you. 13.0 mol Ag x (6.02 x 10^23 atoms Ag/1 mol Ag) = ?? atoms Ag. I assume the second one will be molecules H2O and the third will be Na ions and Cl ions.
Wednesday, January 13, 2010 at 4:40pm by DrBob222

CHEMISTRY
Consider the following cell: Pt|H2(g, 0.130 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 0.90 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion concentration in the anode ...
Friday, May 18, 2012 at 5:45pm by Jematormal91

Chem
For this equation 2 Ag+ (aq) + Cu(s) <--> Cu2+ (aq) + 2 Ag(s) Which occurs at the anode? A. Cu --> Cu2+ + 2e– B. Cu2+ + 2e– --> Cu C. Ag+ + e– -->Ag D. Ag --> Ag+ + e– A, right because it's oxidation?
Friday, May 13, 2011 at 11:12pm by lou

chemistry
I can get you started but it's too long to work out in excruciating detail. AgBr ==> Ag^+ + Br^- Ksp = (Ag^+)(Br^-) = 5.0E-13 When Ag^+ is added ion by ion, AgBr will start to ppt when (Ag^+) = 5.0E-13/0.31 = 1.6E-12. When 99.99% has been pptd that will leave (Br...
Sunday, March 25, 2012 at 3:40pm by DrBob222

Chemistry
a) AgI ==> Ag^+ + I^- Ksp = ? = (Ag^+)(I^-) Substitute Ksp and Ag^+ and solve for I^- In b don't forget to cube the OH^-
Sunday, March 17, 2013 at 11:59pm by DrBob222

Chemistry
I would do this. You have equal volumes of 1.8E-3M NaNO3(which I assume is a typo and you meant AgNO3 AND I assume the small m, meaning molality really is meant to be M or molarity) and 0.2M NaCN. So the concns going into the problem are 9E-4 for Ag^+ and 0.1M for NaCN (just 1...
Thursday, April 7, 2011 at 1:57pm by DrBob222

Chemistry
Ag+2 is generated in a lab. This is an unusual oxidation state for AG. Write the ground state electronic configuration of Ag+2 using the noble gas shortcut.
Thursday, February 23, 2012 at 2:38pm by Drake

Chemistry 219
1.250g x 0.90 = ??g Ag 1.250 x 0.10 = ??g Cu __ Ag| + HNO3 ==> Ag2SO4 Cu| + HNO3 ==> CuSO4 2Ag^+ + Cu(s)(wire) = Ag(s) + Cu^+2(aq) Then Zn(s) + Cu^+2(aq) ==> Zn^+2(aq) + Cu(s) You know grams Ag initially. Convert to moles and use stoichiometry to calculate...
Tuesday, February 8, 2011 at 11:53pm by DrBob222

chemistry
preparation of Ag? determination? Ag can be used as the primary standard for analytical determination of Ag.
Sunday, May 19, 2013 at 2:15am by DrBob222

Chemistry
Consider the following cell: Pt|H2(g, 0.460 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.00 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion concentration in the anode ...
Monday, March 19, 2012 at 4:43pm by Daisy

chemistry
mols Ag = grams/molar mass = ? The coefficients tell you exactly how much NO you get. You get 1 mol NO for every 3 mols Ag; therefore, mols NO = ?mols Ag x (1 mol NO/3 mol Ag) = ?mols x (1/3) = xx mol NO.
Monday, April 9, 2012 at 7:52pm by DrBob222

chemistry
on the reactants, 4 moles nitric to 3 moles silver. calculate the masses in grams to moles for Ag, HNO3. Do you have a 4:3 ratio? If less, then you have excess Ag. If more, then you have Ag as the limiting reagant. so if the ratio is more, then look the ratio of Ag to NO in ...
Tuesday, October 2, 2012 at 6:25pm by bobpursley

Chem
(b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109? % (c) If the mass of Ag-107 is 106.905, what is the mass of Ag-109? amu I really need help. Can u say the answer then explain how you got it? Thanks:)
Sunday, September 26, 2010 at 10:48pm by Rebekah

Chemistry
Mg + 2AgNO3 ==> 2Ag + Mg(NO3)2 mols AgNO3 = M x L mols Ag = mols AgNO3 g Ag = mols Ag x atomic mass Ag.
Tuesday, April 9, 2013 at 6:43pm by DrBob222

chemistry
How many moles Ag are plated. moles = grams/molar mass Ag. How many moles of electrons per mole Ag?
Wednesday, November 30, 2011 at 8:17am by DrBob222

chem
(b) If the natural abundance of Ag-107 is 51.84%, what is the natural abundance of Ag-109? 48.16 % (c) If the mass of Ag-107 is 106.905, what is the mass of Ag-109? 108.9 amu so i got the answers correct but kinda forgot how because it took me a while so do you think you could...
Wednesday, September 29, 2010 at 6:27am by lisa

Chemistry - Equilibrium
mols Ag^+ = 0.05M x 0.500L = 0.025 mols or 0.025/0.505 = 0.02475 M. mols NH3 = 12M x 0.005L = 0.06 mols or 0.06/0.505 = 0.1188 M. ............Ag^+ + 2NH3 ==> Ag(NH3)2^+ Init.....0.025.0.06......0 change-0.025..-0.05..0...025 equil...0......0.010...0.025 equilibrium ...
Wednesday, April 25, 2012 at 4:12pm by DrBob222

Chem
Write the equation and balance it. Colnvet 5.00 g Cu to mols. mols = grams/molar mass Using the coefficients in the balanced equation, convert mols Cu to mols Ag. M Ag = mols Ag/L Ag. You know mols and M, solve for L and convert to mL
Thursday, April 19, 2012 at 8:36pm by DrBob222

chemistry
The solubility products of AgBr and Ag3PO4 are 5.0 10-13 and 1.8 10-18, respectively. If Ag+ is added (without changing the volume) to 1.00 L of a solution containing 0.31 mol Br ‾ and 0.31 mol PO43-, calculate the molarity of Ag+ ions required to initiate ...
Sunday, March 25, 2012 at 3:40pm by Tanner

Chemistry
The Ag electrode gains electrons doesn't it. Ag^+ + e ==> Ag You may be confusing yourself because you have no arrow to show the products versus the reactants. ALWAYS place an arrow in an equation. It isn't an equation without one.
Tuesday, May 10, 2011 at 7:53pm by DrBob222

Science
Try some of the following links: http://search.yahoo.com/search?fr=mcafee&p=theoretical+molar+ratio+values+for+Ag%3ACu+and+Ag%3AAgNO3%3F+ Sra
Friday, May 27, 2011 at 1:27am by SraJMcGin

chemistry
oxidation: Fe2+ --> Fe3+ + e- Reduction: Ag+ +e --> Ag overall is; Fe2+ + Ag+ --> Fe3+ + Ag
Sunday, May 12, 2013 at 3:07pm by bonjo

Chemistry
No, that isn't right; however, I may have led you down the wrong path. I see at the top that the solution is 0.1M in I^- so AgI==> Ag^+ + I^- ........x.....x Ksp = (Ag^+)(I^-) Ag^+ is x from AgI. I^= 0.1M from the problem. 8.51E-17 = (0.1)(x) Solve for x.
Monday, October 29, 2012 at 12:25pm by DrBob222

chemistry
Solid NaI is slowly added to a soln that is 0.010M in Cu+ and 0.010M in Ag+. a. Which compound will begin to precipitate first? b. Calculate [Ag+] when CuI just begins to precipitate/ c. What percent of Ag+ remains in solution at this point?
Monday, July 19, 2010 at 3:13am by Jin

chemistry
Cu + 2AgNO3 ==> 2Ag + Cu(NO3)2 mols Cu = grams/atomic mass Cu Convert mols Cu to mols Ag using the coefficients in the balanced equation. g Ag = mols Ag x atomic mass Ag. This is the theoretical yield.
Thursday, March 7, 2013 at 4:54pm by DrBob222

chemistry
The oxidizing agent, Ag+, gained an electron and is reduced to Ag(s). The reducing agent loses an electron and is oxidized from Fe^2+ to Fe^3+: Ag^+(aq) + Fe^2+(aq) --> Ag(s) + Fe^3+(aq)
Friday, January 1, 2010 at 7:20pm by GK

Chemistry
For a), use Hess' Law. AgCl(s) ==> Ag^+ + Cl^- Ag2CrO4(s) ==> 2Ag^+ + CrO4^-2 b)Since these are equal amounts of NaCl and AgNO3, this will be a saturated solution of AgCl(s) and the solubility is governed by the Ksp for AgCl. AgCl ==> Ag^+ + Cl^- Ksp...
Sunday, October 31, 2010 at 1:42pm by DrBob222

Chemistry
heat lost by Ag turning to solid + heat lost by Ag in heating water + heat gained by water = 0 I don't think you can work this problem unless your are given the melting point of silver. You must know WHERE the initial T is. Perhaps you are to look it up. I did that on the ...
Wednesday, February 24, 2010 at 10:49pm by DrBob222

chemistry
AgI ==> Ag^+ + I^- Ksp = (Ag^+))I^-) Let (AgI) = x, then (Ag^+) = x, then (I^-) = x. Substitute into Ksp and solve for x.
Monday, August 4, 2008 at 6:12pm by DrBob222

Chemistry
AgCl --> Ag^+ + Cl^- AgBr --> Ag^+ + Br^- a. Obviously, AgBr will ppt first because it has the smaller Ksp. (Ag^+)(Br^-) = 7.7 x 10^-13 You know Br^-, you can calculate Ag^+ needed to ppt the first molecule of AgBr. b. Do the same for AgCl to determine the Ag^+ ...
Tuesday, July 27, 2010 at 11:55pm by DrBob222

Chemistry, help!
I answered this question recently. Perhaps it was for another student. First, please clarify if this is 5.0 g Ag or 5.0 g AgNO3. If it is 5.0 g Ag, convert 5.0 g Ag to mols, convert mols Ag to mols Cu using the coefficients in the balanced equation, then convert mols Cu to g ...
Sunday, January 20, 2008 at 10:52am by Anonymous

Ag Science
I have a HUGE project due for ag. It's on California and Hawaii. There are questions like "how many of miles of hiking trail is in the state?" and "how many big game species are in the state?" I am desperately searching all over google for answers to ...
Sunday, March 2, 2008 at 10:25pm by Taylor

Chemistry
Solid NaI is slowly added to a solution that is .010M in Cu+ and .010M in Ag+... a.) which compound will precipitate first b.) calculate [Ag+] when CuI just begins to precipitate c.)what % of Ag+ remains in solution.
Tuesday, September 9, 2008 at 8:12pm by chemstudent

Gen Chem
Consider a cell based on the following reaction: GeO(s) + H2O(l) + 2 Ag+(aq) ===> GeO2(s) + 2 H+(aq) + 2 Ag(s) If [Ag+] = 1 M, at 25°C, would it be..... pH = 2 ( E° - E ) / 0.059159 V. or pH = ( E° - E ) / 0.059159 V.
Friday, March 28, 2008 at 6:02pm by Sarah H

chemistry
"Ag(s) reacts with none of the 4 (solutions of Ag^+2, Pb^+2, Cu^+2, Zn^+2}. So Ag(s) goes at the bottom of the table for now although there may be some metals below silver when you finish with the entire table. Cu(s) reacts with (Ag^+ solution) so Cu goes above Ag ion. It...
Monday, April 14, 2008 at 4:47pm by Joseph

Chemistry
Do you want to work this with equivalents? You know 1 equivalent of Mg = 1 equivalent of Ag = 1 equivalent of anything. That means we will form 4.745 equivalents of Ag. What is the equivalent weight of Ag? 107.9? 4.745 equivalents x 107.9 = ?? g Ag. Note: If you were working ...
Sunday, November 28, 2010 at 4:47pm by DrBob222

chemistry
Ksp AgCl = (Ag^+)(Cl^-) = 1.8 x 10^-10 (Cl^-) = 30.6 mg from the problem. moles Cl = 30.6 x 10^-3 g/35.45 = ??moles and since that is in 1 L of the water sample, that is the molarity. Plug Cl^- (in moles/L) into Ksp and solve for (Ag^+) required for AgCl to ppt. Then M Ag^+ x ...
Wednesday, April 21, 2010 at 8:39pm by DrBob222

chemistry
Fe3+ is added to excess Ag+ prior to titration with KSCN. When all the excess Ag+ has reacted, the red complex of Fe(SCN)2+ forms. This red complex is visible when the [SCN-] is about 2x10^-4M. at this pt. >99% (but not all) of the Ag+ has precipitated. Calc. the Ag+ ...
Tuesday, March 15, 2011 at 7:54pm by emily

AP Chem
AgCl had a mass of 0.1375 g. Change that to mols. mols = g/molar mass AgCl. Convert mols AgCl to mols Ag. That is 1:1. convert mols Ag to grams. grams = mols x molar mass Ag. %Ag = [mass Ag/mass sample]*100 mass sample = 0.1284 g. Post your work if you gt stuck.
Monday, August 27, 2007 at 9:17pm by DrBob222

chem
Right hand side of cell was titrated with Nh3 while monitoring cell voltage: Ag(s)IAg^+ (aq, 0.1 M, 25.0 mL)II Ag^= (aq, 0.1 M, 75.0 mL)I Ag(s) With 1.52 M ammonia titrant, the end point was observed at 9.8 mL. The measured cell voltage was near -0.15 V at the end point. A) ...
Monday, November 24, 2008 at 1:24am by katya

Chemistry
You're right. Since Ag is below Cu in the activity series, Ag will not displace Cu ions. Here is the way you write that. Ag(s) + Cu(NO3)2(aq) ==> no reaction [or you can write NR and most chemists understand that means no reaction.]
Wednesday, March 24, 2010 at 10:22pm by DrBob222

another 12 chem Q. (science)
Moles Ag= Volume*Molarity But moles of Ag has to equal moles of Cl ion (it forms AgCl). Moles Cl=.04*.184*3 (three ions in AlCl3) set them equal, and solve for Volume
Wednesday, February 4, 2009 at 5:15pm by bobpursley

chm
AgIO3 ==> Ag^+ + IO3^- Ksp = (Ag^+)(IO3^-) Solubility AgIO3 = grams/molar mass. Plug that in for Ag^+ and for IO3^- and calculate Ksp.
Sunday, June 27, 2010 at 1:13pm by DrBob222

chemistry
"However, the Ag^+ + I^- reacted to give AgI (but that is not a redox reaction) and if they reacted why didn't Br^- and Ag^+?" Hi Dr.Bob, I am also given additional information for reaction #1 Cu(s) I-(aq) Ag(s) Br- (aq)
Tuesday, April 15, 2008 at 3:28pm by Joseph

chem
heat lost by Ag + heat gained by H2O = 0 [mass Ag x specific heat Ag x (Tfinal-Tintial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0 Substitute and solve for Tfinal which is the only unknown. Then to find heat released, mass Ag x specific heat x delta T (where ...
Sunday, May 20, 2012 at 12:50am by DrBob222

chemistry
q1 = heat to raise T from 130 to 961. q1 = mass Ag x specific heat solid Ag x (Tfinal-Tinitial) [Note: Tfinal is 961). q2 = heat to melt Ag at 961C. q2 = mass Ag x heat fusion. Total q = q1 + q2
Tuesday, October 2, 2012 at 8:53pm by DrBob222

CHEMISRTY
q = mass Ag x specific heat Ag x (Tfinal-Tinitial)
Sunday, April 21, 2013 at 10:45pm by DrBob222

Chemistry
No. I obtained your incorrect answer by NOT squaring (Ag^+). Square the (Ag^+) and you'll be ok.
Sunday, March 17, 2013 at 9:36pm by DrBob222

chemistry
q = mass Ag x specific heat Ag x (Tfinal-Tinitial)
Monday, December 17, 2012 at 3:25pm by DrBob222

CHEMISTRY
Ecell = Eocell - (0.0592/n)log Q Q = (H^+)^2(Ag)^2/pH2*(Ag^+)^2
Friday, May 18, 2012 at 5:45pm by DrBob222

Chemistry Help!!
how many moles of ag contains 4.59*10^25 atoms of Ag
Monday, October 17, 2011 at 4:02pm by Anonymous

Chemistry
You are trying to find [Ag] [Ag]=sqrt 1.1E-12/1.0E-4
Monday, August 10, 2009 at 4:48pm by bobpursley

chemistry
Divide Ksp of one by the other. [KspPbSO4/KspAg2SO4]=[(Pb^+2)(SO4^=)/(Ag^+)^2(SO4^=)]. Note (SO4^=) cancels and you are left with 2*10^-8/1.2*10^-5 = (Pb^+2)(Ag^+)^2 Plug in (Ag^+)^2 and solve for (Pb^+2), Check my thinking.
Monday, May 11, 2009 at 3:52pm by DrBob 222

chemistry
Bob Pursley gave you a hint this morning. Here is another one. Divide Ksp AgCl/Ksp AgI = (Ag^+)(Cl^-)/(Ag^+)(I^&-) = (KspAgCl)/(Ksp AgI). (Ag^+) cancels so you can get a ratio of (Cl^-)/(I^-) = ?? Substitute numbers and solve for (Cl^-)
Wednesday, April 21, 2010 at 5:26pm by DrBob222

Chemistry
For the following electrochemical cell, what is the correct, balanced reaction? Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) A. Cu(s) + Cu2+(aq) → Ag+(aq) + Ag(s) B. Cu(s) + Ag+(aq) → Cu2+(aq) + Ag(s) C. Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) D. Cu2+(aq...
Sunday, March 21, 2010 at 11:49pm by Val

Chemistry
Which one is the LR? Ag or S? 2Ag + S → Ag2S = 216 g Ag + 32 g S
Sunday, March 18, 2012 at 4:08pm by Shea

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